The first step the group took was gather all the information about how electrons and atoms as a whole work before we started figuring out why they have certain properties and trends, like electronegativity. The electrons can have a spin of +½ or -½ causing electron repulsion (amount depends on the group). More electron repulsion on the right side of the periodic table. Those electrons being repelled determine how strong the Zef is because it increases the distance from the nucleus to the valence electrons.
Zef (effective nuclear charge) matters because of the varying electron shielding as you look across the periodic table.The higher the Zef, the stronger it holds on to the electron. Metals tend to have lower Zef’s than nonmetals, interesting enough they are separated by charge (positives are metals and negatives are nonmetals)
Ionic bonds form between metals and nonmetals. The properties of these different atoms must be the reason why they transfer electrons. Covalent bonds have the same charge (negative because they all want to gain electron(s))
For the Trial 1, Atom A has a weak electronegativity and atom B has a stronger electronegativity. The attraction of atom A to atom B is stronger. There was an Ionic Bond Character. For the Trial 2, The electronegativity was made equal for both atoms and the attraction is neutral. There was a nonpolar covalent bond character
For the Trial 3, Increase the electronegativity of atom B and the more electronegative atom (B) is the negatively charge atom. Atom A is positively charged and wants to bond with the negative B atom.
The main observation was if the electronegativity for both atoms is the same or nearly the same, then the bond is covalent. If the electronegativity of any one atom is significantly different, the bond is ionic. A table was created as an example of how atoms ratios of electronegativity matter when determining bond character.
Ratios
Bond
1-10
Ionic Bond
2-3
Covalent Bond
9-9
Covalent Bond
3-8
Ionic Bond
The conclusion that was created was the electronegativity between two or more atoms determines what kind of bond the atoms have. Nonpolar Covalent Bonds result in the same electronegativity, Polar Covalent Bond result in nearly the same electronegativity, while Ionic Bonds result in a big difference of electronegativity. Since metals are located on the left side and nonmetals are on the right, it adds up that they would form ionic bonds, given the huge difference in electronegativity due to ZEF.
The first step the group took was gather all the information about how electrons and atoms as a whole work before we started figuring out why they have certain properties and trends, like electronegativity. The electrons can have a spin of +½ or -½ causing electron repulsion (amount depends on the group). More electron repulsion on the right side of the periodic table. Those electrons being repelled determine how strong the Zef is because it increases the distance from the nucleus to the valence electrons.
Zef (effective nuclear charge) matters because of the varying electron shielding as you look across the periodic table.The higher the Zef, the stronger it holds on to the electron. Metals tend to have lower Zef’s than nonmetals, interesting enough they are separated by charge (positives are metals and negatives are nonmetals)
Ionic bonds form between metals and nonmetals. The properties of these different atoms must be the reason why they transfer electrons. Covalent bonds have the same charge (negative because they all want to gain electron(s))
For the Trial 1, Atom A has a weak electronegativity and atom B has a stronger electronegativity. The attraction of atom A to atom B is stronger. There was an Ionic Bond Character. For the Trial 2, The electronegativity was made equal for both atoms and the attraction is neutral. There was a nonpolar covalent bond character
For the Trial 3, Increase the electronegativity of atom B and the more electronegative atom (B) is the negatively charge atom. Atom A is positively charged and wants to bond with the negative B atom.
The main observation was if the electronegativity for both atoms is the same or nearly the same, then the bond is covalent. If the electronegativity of any one atom is significantly different, the bond is ionic. A table was created as an example of how atoms ratios of electronegativity matter when determining bond character.
The conclusion that was created was the electronegativity between two or more atoms determines what kind of bond the atoms have. Nonpolar Covalent Bonds result in the same electronegativity, Polar Covalent Bond result in nearly the same electronegativity, while Ionic Bonds result in a big difference of electronegativity. Since metals are located on the left side and nonmetals are on the right, it adds up that they would form ionic bonds, given the huge difference in electronegativity due to ZEF.